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Measurements in ChemistryPowerPoint Presentation

Measurements in Chemistry

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Steps in the Scientific Method

- 1. Observations
- - quantitative
- - qualitative
- 2. Formulating hypotheses
- - possible explanation for the observation
- 3. Performing experiments
- - gathering new information to decide
whether the hypothesis is valid

Outcomes Over the Long-Term

- Theory (Model)
- - A set of tested hypotheses that give an
overall explanation of some natural phenomenon.

- Natural Law
- - The same observation applies to many
different systems

- - Example - Law of Conservation of Mass

Law vs. Theory

- A law summarizes what happens
- A theory (model) is an attempt to explain why it happens.

Nature of Measurement

Measurement - quantitative observation

consisting of 2 parts

- Part 1 - number
- Part 2 - scale (unit)
- Examples:
- 20grams
- 6.63 x 10-34Joule seconds

The Fundamental SI Units(le Système International, SI)

SI PrefixesCommon to Chemistry

Uncertainty in Measurement

- A digit that must be estimated is called uncertain. A measurement always has some degree of uncertainty.

Why Is there Uncertainty?

- Measurements are performed with instruments
- No instrument can read to an infinite number of decimal places

Which of these balances has the greatest uncertainty in measurement?

Precision and Accuracy

- Accuracyrefers to the agreement of a particular value with the truevalue.
- Precisionrefers to the degree of agreement among several measurements made in the same manner.

Precise but not accurate

Precise AND accurate

Neither accurate nor precise

Types of Error

- Random Error(Indeterminate Error) - measurement has an equal probability of being high or low.
- Systematic Error(Determinate Error) - Occurs in the same directioneach time (high or low), often resulting from poor technique or incorrect calibration.

Rules for Counting Significant Figures - Details

- Nonzero integersalways count as significant figures.
- 3456has
- 4sig figs.

Rules for Counting Significant Figures - Details

- Zeros
- -Leading zeros do not count as
significant figures.

- 0.0486 has
- 3 sig figs.

Rules for Counting Significant Figures - Details

- Zeros
- -Captive zeros always count as
significant figures.

- 16.07 has
- 4 sig figs.

Rules for Counting Significant Figures - Details

- Zeros
- Trailing zerosare significant only if the number contains a decimal point.
- 9.300 has
- 4 sig figs.

Rules for Counting Significant Figures - Details

- Exact numbershave an infinite number of significant figures.
- 1 inch = 2.54cm, exactly

Sig Fig Practice #1

How many significant figures in each of the following?

1.0070 m

5 sig figs

17.10 kg

4 sig figs

100,890 L

5 sig figs

3.29 x 103 s

3 sig figs

0.0054 cm

2 sig figs

3,200,000

2 sig figs

Rules for Significant Figures in Mathematical Operations

- Multiplication and Division:# sig figs in the result equals the number in the least precise measurement used in the calculation.
- 6.38 x 2.0 =
- 12.76 13 (2 sig figs)

Sig Fig Practice #2

Calculation

Calculator says:

Answer

22.68 m2

3.24 m x 7.0 m

23 m2

100.0 g ÷ 23.7 cm3

4.22 g/cm3

4.219409283 g/cm3

0.02 cm x 2.371 cm

0.05 cm2

0.04742 cm2

710 m ÷ 3.0 s

236.6666667 m/s

240 m/s

5870 lb·ft

1818.2 lb x 3.23 ft

5872.786 lb·ft

2.9561 g/mL

2.96 g/mL

1.030 g ÷ 2.87 mL

Rules for Significant Figures in Mathematical Operations

- Addition and Subtraction: The number of decimal places in the result equals the number of decimal places in the least precise measurement.
- 6.8 + 11.934 =
- 18.734 18.7 (3 sig figs)

Sig Fig Practice #3

Calculation

Calculator says:

Answer

10.24 m

3.24 m + 7.0 m

10.2 m

100.0 g - 23.73 g

76.3 g

76.27 g

0.02 cm + 2.371 cm

2.39 cm

2.391 cm

713.1 L - 3.872 L

709.228 L

709.2 L

1821.6 lb

1818.2 lb + 3.37 lb

1821.57 lb

0.160 mL

0.16 mL

2.030 mL - 1.870 mL

In science, we deal with some very LARGE numbers:

1 mole = 602000000000000000000000

In science, we deal with some very SMALL numbers:

Mass of an electron =

0.000000000000000000000000000000091 kg

Imagine the difficulty of calculating the mass of 1 mole of electrons!

0.000000000000000000000000000000091 kg

x 602000000000000000000000

???????????????????????????????????

Scientific Notation: electrons!

A method of representing very large or very small numbers in the form:

M x 10n

- M is a number between 1 and 10
- n is an integer

. electrons!

2 500 000 000

9

7

6

5

4

3

2

1

8

Step #1: Insert an understood decimal point

Step #2: Decide where the decimal must end

up so that one number is to its left

Step #3: Count how many places you bounce

the decimal point

Step #4: Re-write in the form M x 10n

2.5 x 10 electrons!9

The exponent is the number of places we moved the decimal.

0.0000579 electrons!

1

2

3

4

5

Step #2: Decide where the decimal must end

up so that one number is to its left

Step #3: Count how many places you bounce

the decimal point

Step #4: Re-write in the form M x 10n

5.79 x 10 electrons!-5

The exponent is negative because the number we started with was less than 1.

PERFORMING CALCULATIONS IN SCIENTIFIC NOTATION electrons!

ADDITION AND SUBTRACTION

Review electrons!:

Scientific notation expresses a number in the form:

M x 10n

n is an integer

1 M 10

IF electrons! the exponents are the same, we simply add or subtract the numbers in front and bring the exponent down unchanged.

4 x 106

+ 3 x 106

7

x 106

4.00 x 106

Student A

+ 3.00 x 105

NO!

Is this good scientific notation?

43.00

x 105

=4.300 x 106

To avoid this problem, move the decimal on the smaller number! Make them the same as the largest number.

Direct Proportions

- The quotient of two variables is a constant
- As the value of one variable increases, the other must also increase
- As the value of one variable decreases, the other must also decrease
- The graph of a direct proportion is a straight line

Inverse Proportions

- The product of two variables is a constant
- As the value of one variable increases, the other must decrease
- As the value of one variable decreases, the other must increase
- The graph of an inverse proportion is a hyperbola

Dimensional Analysis

- Dimensional Analysis (also called Factor-Label Method or the Unit Factor Method) is a problem-solving method that uses the fact that any number or expression can be multiplied by one without changing its value. It is a useful technique.
- Unit factors may be made from any two terms that describe the same or equivalent "amounts" of what we are interested in.
- For example, we know that
- 1 inch = 2.54 centimeters

Unit Factors

- We can make two unit factors from this information:inch = 2.54 centimeters

1inch = 2.54 centimeters

2.54 centimeters 1inch

Given units

- When converting any unit to another there is a pattern which can be used.
- Begin with what you are given and always multiply it in the following manner.
- Given units X =Want units
- You will always be able to find a relationship between your two units.
- Fill in the numbers for each unit in the relationship.
- Do your math from left to right, top to bottom.

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